The following initial rate data are for the reaction of mercury(II) chloride with oxalate ion:\[ 2 \text{HgCl}_2 + \text{C}_2\text{O}_4^{2-} \rightarrow 2 \text{Cl}^- + \text{Hg}_2\text{Cl}_2 + 2 \text{CO}_2 \]| Experiment | [HgCl₂]₀, M | [C₂O₄²⁻]₀, M | Initial Rate, M s⁻¹ ||------------|-------------|---------------|----------------------|| 1 | 8.53×10⁻² | 0.378 | 1.26×10⁻⁴ || 2 | 0.171 | 0.378 | 2.52×10⁻⁴ || 3 | 8.53×10⁻² | 0.756 | 5.02×10⁻⁴ || 4 | 0.171 | 0.756 | 1.01×10⁻³ |Complete the rate law for this reaction in the box below. Use the form k[A]^m[B]^n, where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n.Rate = \_\_\_\_\_\_From these data, the rate constant is \_\_\_\_\_\_ M⁻²s⁻¹.

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Chemistry

10th Edition

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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T'he following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution: OCI +I–→ OI + CI Experiment [OCr]o, M T., M 3.23x10-3 Initial Rate, Ms1 1 7.80x10-3 1.78x103 2 7.80x10-3 6.46x103 3.23x10-3 3.57x103 3.57x10-3 7.13x10-3 3 1.56x10-2 1.56x10-2 6.46x10-3 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is Ms1
(c) A reaction between substances R and S was second order with respect to R and second order with respect to S. S-or x 8.1 0.3 At a given temperature, the initial rate of reaction was 1.20 x 10-3 mol dm-3 s-1 when the initial concentration of R was 1.00 x 10-2 mol dm-3 and the initial concentration of S was 2.45 x 10-2 mol dm-3 acom ton Scor 0.8 Calculate a value for the rate constant, k, for the reaction at this temperature. Give the units for k rose ni to nollbeen to stist leitini ert worla of SeldsT otalama) (B) S eldsT amb tom \\ els fallinl Ot *8.1 Inomheqx3
(50,00 Puanlar) 1- Decomposition reaction of ozone (03) in water follows second-order kinetics with a rate constant of 70 M-1sec-1. Assuming that the initial concentration of ozone in water is 1x10-4 M. how many seconds are required for the concentration of ozone to reach 2.5x10-5 M? 015022 92.6 b) 116.9 c) 174.6 265.3 428.6 Boş bırak
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The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH4+NO₂ → N₂ + 2 H₂O Experiment [NH4+]o, M [NO₂ ]o, M Initial Rate, M. s-1 0.0358 1.45 x 10-6 0.0715 0.0358 0.0715 1 2 3 4 Rate = 0.128 0.128 0.255 0.255 Complete the rate law for this reaction in the box below. Use the form k[A]" [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. k = 2.89 x 10-6 2.88 x 10-6 5.76 x 10-6 M-1.s-1
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Use the following data table to answer the following questions. Experiment Concn. of A (M) Concn. of B (M) Initial rate (M/s) 1 0.10 0.010 1.2e-3 2 0.10 0.040 4.8e-3 3 0.20 0.010 2.4e-3 d. The rate constant of the reaction is e. The rate of reaction when concentration of A and B are 0.15M and 0.075M is
The following initial rate data are for the reaction of ICl with hydrogen:2 ICl + H2I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.113 3.10×10-2 1.81×10-4 2 0.226 3.10×10-2 3.63×10-4 3 0.113 6.20×10-2 7.25×10-4 4 0.226 6.20×10-2 1.45×10-3 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k_____ From these data, the rate constant is ______M-2s-1.
The following initial rate data are for the reaction of ICl with hydrogen:2 ICl + H2I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.438 0.105 9.37×10-3 2 0.876 0.105 1.87×10-2 3 0.438 0.209 3.71×10-2 4 0.876 0.209 7.42×10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = _______ From these data, the rate constant is __________M-2s-1.
Doubling the concentration of NO at constant temp is expected to: a.) increase rate by factor of 8 b.) increase rate by factor of 2 c.) doesn't change rate d.) increase rate by factor of 4

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